Method 1: Molar Enthalpies of Reaction, ΔrHm When reactants and products are in their standard state, they are at a pressure of 100 kPa, an aqueous concentration of 1.0 mol/L & liquids and solids are in their pure state. To communicate a molar enthalpy, both the substance & the reaction must be specified.

Formation Reaction Combustion Reaction Note that the above reactions are balanced for one mole of the compound.

Δf Hm° = –239.2 kJ/mol Δc Hm° = –725.9 kJ/mol Formation Reaction CH3OH When 1 mol of methanol is formed from its elements when they are in their standard states at SATP, 239.2 kJ of energy is released. Combustion Reaction Δc Hm° = –725.9 kJ/mol CH3OH The complete combustion of 1 mol of methanol releases 725.9 kJ of energy. Note that the above reactions are balanced for one mole of the compound.

Method 2: Enthalpy Changes, ΔrH Write an enthalpy change (Δr H) beside the chemical equation. CO(g) + 2 H2(g) → CH3OH(l) Δr H = –725.9 kJ The enthalpy change is not a molar value, so does not require the “m” subscript and is not in kJ/mol. Δc H° = –98.9 kJ Δc H° = –197.8 kJ When 2 moles of sulfur dioxide are burned, twice as much heat energy is released as when 1 mole of sulfur dioxide is burned.

Method 3: Energy Terms in Balanced Equations For endothermic reactions, the energy is listed along with the reactants. reactants + energy → products For exothermic reactions, the energy is listed along with the products. reactants → products + energy

Method 4: Chemical Potential Energy Diagrams During an exothermic reaction, the enthalpy of the system decreases. Heat flows out of the system and into the surroundings & we observe a temperature increase.

Method 4: Chemical Potential Energy Diagrams During an endothermic reaction, the enthalpy of the system increases. Heat flows into the system from the surroundings & we observe a temperature decrease.

Summary

Homework: Read pgs. 495 – 500 Section 11.3 Questions #’s 1, 3, 4, 5 (p. 501)